What Is Strontium Definition Atomic Number Electronic Configuration Reactions and Uses
The chemical name of Sr is Strontium. Strontium is an element having an atomic number of 38 and atomic mass 87.62 g.mol-1. By nature, Strontium is an alkaline earth metal. Owing to its electronic configuration, Sr element has some specific properties and happens to be highly reactive. It is an alkaline earth metal and is yellowish and silver-white. The metal also reacts with air to produce a dark oxide layer. Physically and chemically, the Sr element is similar to its neighbours on the periodic table—Calcium and barium. Strontium was discovered collaboratively by Adair Crawford and William Cruikshank in 1790.
Sr Chemical Nature
The chemical nature of Strontium is very reactive. In the periodic table, Strontium belongs to group 2. It has a high melting point of 777°C or 1431°F or 1050 K. Strontium belongs to period five and has a boiling point of 1377°C or 2511°F or 1650 K. The density of Sr element (where Sr is the chemical symbol for Strontium) is 2.64 g cm3 and is in the block s of the periodic table. With an atomic number of 38, the relative atomic mass of Strontium is 87.62. The metal has four isotopes--84Sr, 86Sr, 87Sr, 88Sr. Strontium's electronic configuration [Kr] 5s and CAS number 7440-24-6.
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Uses of Strontium
Sr, in chemistry, has many applications. Typical uses of Strontium are listed below:
In Television
Sr chemical name Strontium has the most important application in the production of glass manufacture of cathode ray tubes found in colour television. However, this use of Sr element is gradually on the decline owing to the declining usage of CRTs in televisions. This has consequently significantly affected the way Strontium is mined and refined.
In Fireworks
Strontium is used to create Strontium Carbonate and other Strontium salts which are used to give red colour to fireworks. This property also helps to distinguish Strontium from other elements in a flame test. The production of fireworks constitutes 5 percent of the world's total output.
In Biology and Medicine
Strontium is present in varied quantities in all living organisms. Since Strontium is quite similar to the element calcium, it is located in bones. In Europe and Australia, Strontium ranelate, which is a pharmacologic agent, is used to treat osteoporosis in individuals. However, this method is not allowed in Canada or the United States. In orthopaedic surgery, injectable acrylic bone cement is commonly used to treat prostheses. For arthroplasties of the knee, hip and other joints and fixation of metallic or polymer prosthetics implants to bones, Conventional polymethylmethacrylate (PMMA) is used. However, this method still suffers from certain drawbacks such as a high exothermic reaction and poor attachment of bone cement to the bone surface.
In Geology
Strontium, owing to its strong association with calcium, is very useful in indicating the presence of calcareous rocks, especially those associated with Mg and Ba. In places where Ca, along with other elements give an indication of calcareous rocks and felsic intrusive indicated by other elements, the bedrock geology would be favourable for different elements.
Properties of Strontium
Strontium's atomic number is 38, and Sr's atomic mass is 88. The Sr element (chemical name strontium) has four isotopes which are naturally occurring out of which 88Sr is most commonly found in nature. Chemically there are similarities between Strontium and other heavier alkaline earth metals such as Barium and Calcium. Strontium has a vigorous reaction with water and tarnishes and tarnishes rapidly in air. Strontium is commonly found combined with other elements and compounds owing to the highly reactive nature of the element. Strontium which has been turned into fine powder will ignite spontaneously in air and result in the formation of Strontium nitride and Strontium Oxide. Sr is a metallic lithophile element. An ion of Sr2+ has a size of 118pm which is in between the sizes if calcium ion (100pm) and potassium ion (138pm) and readily substitutes in a large number of minerals which are rock-forming like dolomite, calcium, gypsum, plagioclase and K-feldspar. Sr minerals are comparatively rare, but some of them are SrCO3 and SrSO4, which are included in pegmatites or hydrothermal deposits.
Did You Know?
Here's a very interesting Strontium element fact . Although naturally occurring Strontium (strontium-88) is stable, the Strontium-90 which is synthetic is very radioactive. Strontium-90 is one of the most harmful aspects of nuclear fallout. This is because the human body absorbs Strontium like Calcium. Naturally occurring stable Strontium does not harm us. Owing to the high reactivity of Strontium, it usually occurs only in the form of compounds.
FAQs on Strontium Element Chemistry Properties and Applications
1. What is strontium in chemistry?
Strontium (Sr) is a chemical element with atomic number 38 that belongs to the alkaline earth metals (Group 2) of the periodic table. It is a soft, silvery metal that is highly reactive and forms compounds mainly in the +2 oxidation state (Sr2+). Strontium is found naturally in minerals such as strontianite (SrCO3) and celestine (SrSO4). Because of its reactivity, it is usually stored under oil to prevent reaction with air and moisture.
2. What is the electron configuration of strontium?
The electron configuration of strontium (Sr) is [Kr] 5s2. This means:
- It has 38 electrons in total.
- The core configuration is the noble gas krypton (Kr).
- It has two valence electrons in the 5s orbital.
3. What is the oxidation state of strontium?
The most common and stable oxidation state of strontium is +2. Strontium loses its two 5s valence electrons to form the ion Sr2+. For example, in strontium chloride (SrCl2), strontium has a +2 charge and each chloride ion is Cl-. The +2 oxidation state is characteristic of all Group 2 alkaline earth metals.
4. How does strontium react with water?
Strontium reacts with water to form strontium hydroxide and hydrogen gas. The balanced chemical equation is:
Sr(s) + 2H2O(l) → Sr(OH)2(aq) + H2(g).
- This reaction is exothermic.
- Strontium hydroxide is a strong base.
- The reaction becomes more vigorous down Group 2 compared to magnesium.
5. What color does strontium produce in a flame test?
Strontium produces a bright red (crimson) flame in a flame test. This red color is due to the excitation of electrons in Sr2+ ions, which emit red light when they return to lower energy levels. Because of this property, strontium salts such as Sr(NO3)2 are widely used in fireworks and signal flares to produce red colors.
6. What are the main uses of strontium in chemistry and industry?
Strontium is mainly used in fireworks, ceramics, magnets, and medical imaging. Key applications include:
- Strontium nitrate (Sr(NO3)2) in red fireworks.
- Strontium ferrite in permanent magnets.
- Strontium aluminate in glow-in-the-dark materials.
- Strontium-89 in medical treatment for bone cancer pain.
7. What is strontium carbonate used for?
Strontium carbonate (SrCO3) is used mainly in ceramics, glass production, and pyrotechnics. It is:
- A raw material for making other strontium compounds.
- Used in special glass for color and durability.
- A component in fireworks to help produce red flames.
8. What is the difference between strontium and calcium?
Strontium and calcium are both Group 2 alkaline earth metals, but strontium is larger and more reactive. Key differences include:
- Atomic number: Calcium = 20, Strontium = 38.
- Atomic radius: Strontium is larger due to more electron shells.
- Reactivity: Strontium reacts more vigorously with water.
- Flame test: Calcium gives orange-red, strontium gives bright red.
9. How is strontium extracted from its ores?
Strontium is extracted mainly from celestine (SrSO4) by converting it to strontium carbonate and then reducing it. The process involves:
- Reduction of SrSO4 with carbon to form SrS.
- Reaction of SrS with CO2 to produce SrCO3.
- Conversion to strontium oxide (SrO) and reduction with aluminum:
3SrO(s) + 2Al(s) → 3Sr(g) + Al2O3(s).
10. What is strontium-90 and why is it important?
Strontium-90 (Sr-90) is a radioactive isotope of strontium produced in nuclear fission with a half-life of about 28.8 years. It undergoes beta decay to form yttrium-90. Because Sr2+ behaves chemically like Ca2+, it can accumulate in bones if ingested, making it a significant radiological hazard. Sr-90 is also used in radioisotope thermoelectric generators and scientific research.
